A) \[\text{MS}{{\text{O}}_{\text{4}}}\text{.}{{\text{H}}_{\text{2}}}\text{O}\]
B) \[{{\text{M}}_{\text{2}}}\text{S}{{\text{O}}_{\text{4}}}\text{.2}{{\text{H}}_{\text{2}}}\text{O}\]
C) \[{{\text{M}}_{\text{2}}}\text{S}{{\text{O}}_{\text{4}}}\text{.3}{{\text{H}}_{\text{2}}}\text{O}\]
D) \[\text{MS}{{\text{O}}_{\text{4}}}\text{.5}{{\text{H}}_{\text{2}}}\text{O}\]
Correct Answer: D
Solution :
As the metal is divalent, the formula of hydrated sulphate will be \[\text{MS}{{\text{O}}_{\text{4}}}\text{.x}{{\text{H}}_{\text{2}}}\text{O}\] To find the value of x: 0.10 mol of \[\text{MS}{{\text{O}}_{\text{4}}}\] combines with 9 g of \[{{\text{H}}_{\text{2}}}\text{O}\] (i.e., 0.5 mol of water). \[\left[ \because \text{moles of }{{\text{H}}_{2}}O=\frac{9}{18}=0.5 \right]\] \[\therefore 1\text{ mol}\]of \[\text{MS}{{\text{O}}_{\text{4}}}\] will combine with \[\frac{0.5}{0.10}=5\text{ mol}\] of water. So, formula of sulphate is \[\text{MS}{{\text{O}}_{\text{4}}}\text{.5}{{\text{H}}_{\text{2}}}\text{O}\].
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